1
Knowledge and Understanding [45]
Put your answer, in capitol letters, for each multiple choice question in the blank at the beginning of each question.
Unit #1 B Matter and Chemical Bonding [15]
- ____ The scientist who developed the Abilliard ball@ model of the atom was
a) Ernest Rutherfordb) J. J. Thomsonc) John Daltond) Niels Bohr
- ____ The scientist who is credited with the discovery of the nucleus from his gold foil experiment is
a) Ernest Rutherfordb) J. J. Thomsonc)John Daltond) Niels Bohr
- ____ The mass number of an element represents the quantity of which subatomic particles in an atom?
a) protons and electronsc) electrons and neutrons
b) protons and neutronsd) protons, electrons, and neutrons
- ____ How many elements in the main body of the Periodic Table are liquids at room temperature (25oC)?
a) 2b) 5c) 11d) 15
- ____ Isotopes of an element have differing numbers of
a) electronsb) neutronsc) protonsd) energy levels
- ____ Which of the following elements does not exist as a diatomic molecule in its natural state?
a) hydrogenb) sodiumc) oxygend) nitrogen
- ____ An anion is an element that has
a) gained protonsb) lost protonsc) gained electronsd) lost electrons
- ____ Which ion does not have the same number of electrons as argon?
a) Ca2+b) Al3+c) S2-d) Cl1-
- ____ Arsenic belongs to which family of elements?
a) alkali metalsb) alkaline metalsc) metalloidsd) transition metals
- ____ Iodine belongs to which family of elements?
a) metalloidsb) noble gasesc) halogensd) man-made
- ____ The amount of energy required to remove an electron from an atom is its
a) electronegativityb) ionization energyc) electron affinityd) cation energy
- ____ To create an ionic bond with a non-metal atom, a metal atom must do what?
a) gain electronsb) lose electronsc) share electronsd) any of these
- ____ What do the springs in the molecular model sets represent?
a) a pair of shared valence electronsc) valence electrons from one atom only
b) a pair of shared core electrons d) core electrons from one atom only
- ____ Which of these compounds will not likely dissolve well in water?
a) sodium nitrateb) silver bromidec) barium hydroxided) copper (II) sulfate
- ____ Which of the following is an example of a binary acid?
a) HClb) HClO3c) H2SO4d) CH3COOH
Unit #2 B Chemical Reactions [5]
- ____ Which chemical equation is properly balanced for the formation of water from its elements?
a) H2 + O2 H2Ob) H2 + O H2Oc) H2 + O2 2H2Od) 2H2 + O2 2H2O
- ____ Which type of chemical reaction always has only one reactant and more than one product formed?
a) synthesisb) decompositionc) single replacementd) combustion
- ____ Which type of chemical reaction always has an element and a compound on each side of the equation?
a) synthesisb) decompositionc) single replacementd) combustion
- ____ The most undesirable product in incomplete combustion reactions is
a) waterb) carbon monoxidec) carbon dioxided) oxygen
- ____ The reaction between a metal oxide, such as MgO, and water will result in the formation of
a) a baseb) an acidc) hydrogend) oxygen
Unit #3 B Quantities in Chemical Reactions [10]
- ____ The atomic mass of an element represents
a) the mass, in grams, of one mole of atomsc) the number of moles of one gram of atoms
b) the mass, in grams, of a sample of atomsd) the number of particles in a mole of atoms
- ____ How many moles is equivalent to 5.58 x 1020 molecules of propane gas (C3H8)?
a) 1.27 x 1019b) 1.08 x 103c) 4.41 x 101d) 9.27 x 10-4
- ____ What is the mass of 2.31 moles of table salt (sodium chloride)?
a) 0.0395 gb) 2.31 gc) 58.44 gd) 135.00 g
- ____ How many formula units are there in a mole of Ca3P2?
a) 1b) 2c) 3d) 6.02 x 1023
- ____ How many molecules are there in a 32 g sample of oxygen gas?
a) 16b) 32c) 6.02 x 1023d) 1.20 x 1024
- ____ A compound with a mass of 48.72 g is found to contain 16.03 g of sulfur and the remaining mass is zinc. What is the percentage composition of zinc in the compound?
a)67%b) 49%c) 34%d) 33%
- ____ What is the percentage composition of oxygen in a carbon dioxide molecule?
a) 27%b) 33%c) 66%d) 73%
- ____ Ammonia gas can be synthesized using this equation: N2(g) + 3 H2(g) 2 NH3(g)
If 4 moles of nitrogen gas are available for the reaction, how many moles of ammonia will be produced?
a) 4b) 6c) 8d) 12
- ____ The calculated mass of a product from the initial mass of a limiting reactant is called the
a) theoretical massb) actual massc) molar massd) percentage mass
- ____ It is calculated that a reaction should produce 12.5 g of a product but only 9.9 g is produced. The percentage yield of the reaction is
a) 13%b) 21%c) 26%d) 79%
Unit #4 B Solutions and Solubility [10]
- ____ Which factor has very little effect on increasing the rate of dissolving a solid solute in a liquid solvent?
a) increasing temperatureb) agitation (stirring)c) decreasing particle sized) increasing pressure
- ____ What happens to the solubility of a gas in water as the temperature of the solution increases?
a) it increasesb) it decreasesc) it is not affected
- ____ Solubility curves are graphs
a) that always have linear relationshipsc) representing unsaturated solutions only
b) of grams of solute per 100mL of water vs. temperatured) all of these
- ____ A rubbing alcohol bottle from the drugstore reads A60% v/v@. The volume of the bottle is 500 mL. What is the volume of alcohol in the bottle?
a) 30 mLb) 60 mLc) 200 mLd) 300 mL
- ____ Water supplies may not contain more than 500 ppm of calcium carbonate. What is the maximum mass, in mg, of calcium carbonate that is acceptable in a cup of tap water (0.250 L)?
a) 0.01 mgb) 0.1mgc) 10 mgd) 100 mg
- ____ An Arrhenius base is a compound that dissociates to produce
a) OH- ionsb) H+ ions c) H2Od) Na+ ions
- ____ Which of the following is not a characteristic of an acid?
a) reacts with carbonates to produce CO2c) feels like water to the touch
b) reacts with most metals to produce H2d) all of these are characteristics of acids
- ____ As an acid is diluted, what happens to its pH value?
a) it increasesb) it decreasesc) it is unaffectedd) it cannot be predicted
- ____ The hydronium ion concentration of a solution is 5.67 x 10-4. What is its pH?
a) 3.25b) 4.75c) 5.67d) 10.75
- ____ The pH of citrus fruits, like oranges and lemons, is closest to
a) 1b) 3c) 7d) 10
Unit #5BGases and Atmospheric Chemistry [5]
- ____ The air we breathe consists of what percentage of oxygen?
a) 10%b) 15%c) 21%d) 78%
- ____ What happens to the air pressure in the atmosphere as altitude increases?
a) it increasesb) it decreasesc) it does not change
- ____ What is the temperature at “absolute zero”?
a) 0oCb) 0oFc) 0oKd) all of these
- How many kilopascals is equivalent to 1.21 atm?
a) 83.7 kPab) 101.3 kPac) 123 kPad) 919.6 kPa
- Jacques Charles is credited for discovering what relationship for ideal gases?
a) temperature varies directly with pressurec) volume varies directly with temperature
b) pressure varies inversely with volumed) the molar volume of a gas at STP is 22.4 L per mole
1
Thinking and Inquiry[40]
Answer all questions in this section on foolscap except for T3.
Unit #1 B Matter and Chemical Bonding [12]
T1.As strange as it first appears looks, you have learned this year that the Periodic Table of Elements has quite a number of relationships between elements in its columns and rows that are sensible and predictable. Choose 3 trends that exist in the columns and/or rows of the Periodic Table to explain the “Perioidicity”, or patterning,of the Periodic Table of Elements. You may find a T-chart useful in organizing your answer. [6]
T2.In this course, you have learned about the formation of ionic and molecular compounds from elements. Use a T-chart to compare and contrast these compounds using 3 criteria of your choice. You may consider, but are not limited to, the types of elements in each, naming rules, the bonding that forms, physical properties, etc. [6]
Criteria / Ionic Compound / Molecular CompoundUnit #2 B Chemical Reactions [8]
T3.i)Fill in the product(s) formed in each reaction where possible in the space provided. If no reaction occurs, write ANR@ for the products. [5]
ii)Where a reaction takes place, balance the equation if it is not balanced already. [3]
a)MgCl2(s)
b)C5H12(l) + O2(g)
c)I2(g) + LiF(aq)
d)Zn(s) + O2(g)
e) Al(s) + AuNO3(aq)
Unit #3 B Quantities in Chemical Reactions [9]
T4.Ammonia gas can be produced in the laboratory by heating ammonium chloride with calcium hydroxide according to the following balanced equation:
2 NH4Cl(s) + Ca(OH)2(s) CaCl2(s) + 2 NH3(g) + 2 H2O(g)
In this reaction 8.93 g of ammonium chloride is heated with 7.48 g of calcium hydroxide. Determine which reactant is limiting and calculate the theoretical mass of ammonia gas produced in this reaction. [6]
T5.A chemistry student becomes very frustrated when his percentage yields are not 100% (he is a perfectionist!). Suggest three detailed reasons why the percentage yield of his reactions might not be exactly 100%. [3]
Unit #4 B Solutions and Solubility [7]
T6.While cleaning out the chemical storage room at the end of the semester, Ms. Gerber discovers a bottle of hydrochloric acid that has no concentration label on it. Practising what she preaches, she mixes up a standard solution of 0.250 mol/L sodium hydroxide and carries out a perfect titration: a 15.00 mL sample of the acid requires 23.94 mL of the base to reach the endpoint.
a)Write a balanced equation for this reaction. [1]
b) Calculate the concentration of hydrochloric acid in the mystery bottle. [4]
T7.Explain how the strength of an acid is different from its concentration. Include an example. [2]
Unit #5BGases and Atmospheric Chemistry [4]
T8.Neon gas is widely used as the luminous gas in signs around Goderich. A sample of neon has a volume of 5.5 L at 750 torr at 10.0°C. If the gas is expanded to a volume of 7.5 L at a pressure of 400 torr, what will its final temperature be (in °C)? [4]
Application [45]
Answer all questions in this section on the exam paper (except for A4) on foolscap.
Unit #1 B Matter and Chemical Bonding [15]
A1.Show how chlorine can take part in an ionic bond, a pure covalent bond, and a polar covalent bond. [3]
A2.Draw a Lewis structure for CS2. [2]
A3.The isotopic abundance for Silicon is: 92.21% Si-28; 4.70% Si-29; and 3.09% Si-30. Use this data to calculate the average atomic mass of silicon. [2]
A4.Fill in the table for the following ionic and molecular substances. [8]
IUPAC Name / Chemical Formulaaluminum sulfide
(Provide IUPAC Name
and Classical Name) / Fe(OH)3
NaHCO3
nickel (II) chloride hexahydrate
(Provide Ionic Name
and Acid Name) / HClO2
carbon tetrachloride
Unit #2 B Chemical Reactions [8]
A5.A 3U chem student sees a bottle of calcium chloride solution and a bottle of sodium carbonate solution on a lab bench in Lab 2 and decides to see what happens if these two solutions are mixed together in a test tube (maybe they=ll blow up!!!). Instead, the formation of a white precipitate is observed. : (
a) Write a balanced equation for the reaction and indicate which product is the precipitate. [5]
b) Write the total ionic and net ionic equations for the reaction. [2]
c) Identify the two spectator ions in the reaction. [1]
Unit #3 B Quantities in Chemical Reactions [10]
A6.How many atoms of carbon are contained in a 500 mg tablet of pure vitamin C (C6H8O6)? [4]
A7.Vanillin, the compound responsible for the flavour vanilla, has a molar mass of 152.16 g/mol. The percentage composition of vanillin is 63.2% carbon, 5.26% hydrogen, and 31.6% oxygen. Determine whether its molecular formula is the same as its empirical formula. [6]
Unit #4 B Solutions and Solubility [8]
A8.In preparing for next semester=s science classes, Ms. Gerber=s asks you to spend your PD day in Lab 2 as her lab assistant. She gives you a 6 mol/L bottle of sulfuric acid and tells you to use it to make 2 L of a 0.5 mol/L solution. Explain how you would do this and include any necessary calculations in your response. [4]
A9.Run down and tired from studying for your chemistry exam, you decide to make 500 mL of a 1.5 mol/L sugar solution (sucrose = C12H22O11) to drink right before writing the exam for an instant Aenergy boost@. Explain how you would do this and include any necessary calculations in your response. [4]
Unit #5BGases and Atmospheric Chemistry [4]
A10.What volume does 1.50 g of nitrogen gas occupy at 100.0oC and 5.00 atm? [3]
You=re Finished!
Best of luck to you in all your future endeavours. It has been a pleasure teaching you this semester.
Keep in touch and perhaps I=ll see you in 4U Chemistry!
1
Goderich District Collegiate Institute
SCH 3U (Grade 11 University Chemistry)
Friday, January 27, 2012
9:00 am -- 11:00 am
Lab 2
Aids Permitted (supplied by student):
- Pens and pencils
- Scientific calculator
- Foolscap as required
- ALCHEM Periodic Table of Elements and Ions
Student Name: ______
Student Instructions:
- Make sure your name is on every piece of paper to be submitted.
- Answer foolscap questions on one side of the paper only and do not mix questions from different parts of the exam on a page.
- Refer to the bottom of this page for given information to use in your calculations.
- Read all questions carefully, noting their mark values and using your allotted time appropriately. Completion of the exam using “a mark a minute” is an excellent guide.
- There is no penalty for incorrect answers so attempt every question.
- No electronic devices of any kind, aside from a non-programmable calculator, are permitted during the exam. Cell phones must be turned “OFF” and not be present on your person.
- Read over and check your answers thoroughly when you are finished the exam before submitting the entire exam to the supervising teacher.
- Communication will be assessed using the following rubric:
Communication Rubric / Level 1 / Level 2 / Level 3 / Level 4
Communication of information and ideas / Communicates information and ideas with limited clarity and precision / Communicates information and ideas with some clarity and precision / Communicates information and ideas with considerable clarity and precision / Communicates information and ideas clearly and precisely
Use of scientific terminology, S.I. units, and significant digits / Uses scientific terminology, S.I. units, and significant digits with limited accuracy / Uses scientific terminology, S.I. units, and significant digits with some accuracy / Uses scientific terminology, S.I. units, and significant digits with minor misuse / Uses scientific terminology, S.I. units, and significant digits with very few errors
- This examination is the property of the Science Department at GDCI.
Given Information
NA = 6.02 x 1023 particles per molen = m / M
n = N / NA
n = C x V
ppm = mass of solute (mg)
volume of solution (L)
= mass of solute (g) x 1 x 106
mass of solution (g)
density of water = 1 g per mL
CiVi = CfVf
pH = -log10[H+ ]
na x Cb x Vb = nb x Ca x Va
OoC = 273.15 K
P1V1 = P2V2
T1 T2
PV = nRT
R = 8.314 (kPa x L)/(K x mol)
1 atm = 760 mm Hg = 760 torr = 101.3 kPa = 14.7 psi / Activity Series
(most reactive)
lithium
potassium
barium
calcium
sodium
magnesium
alumnium
zinc
chromium
iron
cadmium
cobalt
nickel
tin
lead
hydrogen
copper
mercury
silver
platinum
gold
(least reactive)